Question

) Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2is 7.78 × 10-1M/s, what is the rate of the loss of O3

Answer 1

Rate of the reaction is 0.2593 M/s

-0.5186 M/s is the rate of the loss of ozone.

Step-by-step explanation:

The rate of the reaction is defined as change in any one of the concentration of reactant or product per unit time.

`2O_3\rightleftharpoons 3O_2`

Rate of formation of oxygen :
`7.78* 10^(-1) M/s`

Rate of the reaction(R) =
`(-1)/(2)(d[O_3])/(dt)=(1)/(3)(d[O_2])/(dt)`

`R=(1)/(3)(d[O_2])/(dt)`

Rate of formation of oxygen=3 × (R)

`7.78* 10^(-1) M/s=3* R`

Rate of the reaction(R):
`0.2593 M/s`

Rate of the reaction is 0.2593 M/s

Rate of disappearance of the ozone:

`R=-(1)/(2)(d[O_3])/(dt)`

`(d[O_3])/(dt)=-2* R=-2* 0.2593* M/s=-0.5186M/s`

-0.5186 M/s is the rate of the loss of ozone.